Under standard-state conditions, which of the following species is the best reducing agent? a. ag+ b. pb c. h2 d. ag e. mg2+

The correct answer is Option b.

Explanation:

Reducing agents are defined as the agents which help the other substance to get reduced and itself gets oxidized. They undergo oxidation reaction.

For determination of reducing agents, we will look at the oxidation potentials of the substance. Oxidation potentials can be determined by reversing the standard reduction potentials.

For the given options:

This ion cannot be further oxidized because +1 is the most stable oxidation state of silver.

This metal can easily get oxidized to ion and the standard oxidation potential for this is 0.13 V

This metal can easily get oxidized to ion and the standard oxidation potential for this is 0.0 V

This metal can easily get oxidized to ion and the standard oxidation potential for this is -0.80 V

This ion cannot be further oxidized because +2 is the most stable oxidation state of magnesium.

By looking at the standard oxidation potential of the substances, the substance having highest positive potential will always get oxidized and will undergo oxidation reaction. Thus, considered as strong reducing agent.

From the above values, the correct answer is Option b.

answer; 4 electrons;

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